Which one of the following statements is false

Options

A. The electron affinity of chlorine is less than that of fluorine
B. The electronegativity of fluorine is more than that of chlorine
C. The electron affinity of bromine is less than that of chlorine
D. The electronegativity of chlorine is more than that of bromine

Explanation

To determine which statement is false regarding the electron affinity of chlorine and fluorine, we need to analyze the properties of these elements based on their position in the periodic table and their electron affinity values.

### Step-by-Step Solution:

1. **Understanding Electron Affinity**:
- Electron affinity is defined as the amount of energy released when an electron is added to a neutral atom in the gas phase. It is a measure of how much an atom wants to gain an electron.

2. **Position in the Periodic Table**:
- Chlorine (Cl) is located in Group 17 (the halogens) of the periodic table, while Fluorine (F) is also in Group 17 but is higher in the group.

3. **Trends in Electron Affinity**:
- Generally, as we move up a group in the periodic table, the electron affinity tends to increase due to the decrease in atomic size and increase in effective nuclear charge. However, this trend can have exceptions.

4. **Comparing Chlorine and Fluorine**:
- Fluorine is expected to have a higher electron affinity than chlorine due to its higher electronegativity. However, the small size of fluorine leads to significant electron-electron repulsion when an additional electron is added, which can reduce the energy released during this process.

5. **Conclusion on the False Statement**:
- The statement that "the electron affinity of chlorine is less than that of fluorine" is false. In reality, chlorine has a higher electron affinity than fluorine due to the repulsion experienced in fluorine when an electron is added.

### Final Answer:
The false statement is: "The electron affinity of chlorine is less than that of fluorine."

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